How many grams of CO2 and grams of H2O are produced when 52.0 g C2H2 burns in oxygen?
Answers
2C2H2 + 5O2 --> 4CO2 + 2H2O
1 mole of C2H2 = 2 (12.0) + 2(1.0) = 26.0 g
1 mole of CO2 = 12.0 + 2 (16.0) = 44.0 g
1 mole of H2O = 2(1.0) + 16.0 = 18.0 g
52 g C2H2 x 1 mol / 26 g = 2.0 mol C2H2
2.0 mol C2H2 x 4 CO2 / 2 C2H2 = 4.0 mol CO2
4.0 mol CO2 x 44.0 g / mol = 176 g CO2
52 g C2H2 x 1 mol / 26 g = 2.0 mol C2H2
2.0 mol C2H2 x 2 H2O / 2 C2H2 = 2.0 mol H2O
2.0 mol H2O x 18.0 g / mol = 36 g H2O
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Answer:
88 grams of CO₂ and 36 grams of H₂O are produced when 52.0 g of C₂H₂ burns in oxygen.
Explanation:
Molar mass of C₂H₂ = 12×2 + 1×2
= 26 g/mol
The number of moles is calculated by using the formula,
n = given mass/molar mass
The number of moles of C₂H₂= 52/26
= 2 moles
2 moles of C₂H₂ ⇒ 4 moles of CO₂.
The molar mass of carbon dioxide is 44 g/mol.
Mass of CO₂ = 44×4
= 176 g
2 moles of C₂H₂ ⇒ 2 moles of H₂O.
The molar mass of water is 18 g/mol.
Mass of H₂O = 18×2
= 36 g
Thus, 176 grams of CO₂ and 36 grams of H₂O are produced when 52.0 g of C₂H₂ burns in oxygen.
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